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grandymaker [24]
3 years ago
13

A water sample tested positive for lead with a concentration of 35 ppm. The density of the solution is 1.00 g/mL Which of the fo

llowing statements is correct?
A. 100 g of the solution contains 35 g of lead
B. there are 35 mg of lead in 1.0 L of this solution
C. 100 g of the solution contains 35 mg of lead
D. the solution is 35% by mass of lead
E. Ethe molarity of the solution is 35 M
Chemistry
1 answer:
Nimfa-mama [501]3 years ago
4 0

Answer: option B. there are 35 mg of lead in 1.0 L of this solution

Explanation:

1ppm = 1mg/L

Therefore 35ppm = 35mg/L

So, the solution contains 35mg of lead in 1L of the solution

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1s² 2s¹
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How many atoms are needed to react with 50 grams of O2 gas
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3 moles

Explanation:

3 moles atoms are needed to react with 50 grams of O2 gas.

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At a particular temperature a 2.00-L flask at equilibrium contains 2.80 ✕ 10-4 mol N2, 2.50 ✕ 10-5 mol O2, and 2.00 ✕ 10-2 mol N
zhenek [66]

Answer : The value of equilibrium constant (K) is, 5.71\times 10^4

Explanation :

First we have to calculate the concentration of N_2,O_2\text{ and }N_2O

\text{Concentration of }N_2=\frac{\text{Moles of }N_2}{\text{Volume of solution}}=\frac{2.80\times 10^{-4}mol}{2.00L}=1.4\times 10^{-4}M

and,

\text{Concentration of }O_2=\frac{\text{Moles of }O_2}{\text{Volume of solution}}=\frac{2.50\times 10^{-5}mol}{2.00L}=1.25\times 10^{-5}M

and,

\text{Concentration of }N_2O=\frac{\text{Moles of }N_2O}{\text{Volume of solution}}=\frac{2.00\times 10^{-2}mol}{2.00L}=1.00\times 10^{-2}M

Now we have to calculate the value of equilibrium constant (K).

The given chemical reaction is:

N_2(g)+O_2(g)\rightarrow 2N_2O(g)

The expression for equilibrium constant is:

K=\frac{[N_2O]^2}{[N_2][O_2]}

Now put all the given values in this expression, we get:

K=\frac{(1.00\times 10^{-2})^2}{(1.4\times 10^{-4})\times (1.25\times 10^{-5})}

K=5.71\times 10^4

Thus, the value of equilibrium constant (K) is, 5.71\times 10^4

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3 years ago
Which statement best explains the change in the matter before and after the change?
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What is the pressure of the dry gas alone ?
gtnhenbr [62]

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<h3>Further explanation</h3>

Given

P tot=760 torr

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Required

P gas/O₂

Solution

Dalton's law of partial pressures stated that

<em>the total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases   </em>

Can be formulated:  

P tot = P1 + P2 + P3 ....  Pn

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760 torr = 23.8 torr + P O₂

P O₂ = 760 - 23.8

P O₂ = 736.2 torr

3 0
3 years ago
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